Thursday, March 4, 2010

Here is the AP equation sheet with equations and constants that you will have available to you on the winter exam.

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The exam covers material from chapters 6 through 9.

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Chapter 6

1. define energy and temperature
2. calculate heat (q) using mCDT equation
3. writing thermochemical equations
4. sign of DH for endothermic and exothermic reactions
5. stoichiometry calculations with thermochemical equations
6. Hess's law of heat summation (find DH for a reaction using Hess's law)
7. standard enthalpy of formations (find DH for a reaction using summation of product enthalpies - summation of reactant entalpies)

Chapter 7

1. Properties of light
   1. be able to calculate wavelength, frequency, and energy of photons of light (equations and constants are given on the equation sheet)
   2. know the type of electromagnetic radiation from low energy to high energy: radio, micro, infrared, visible, ultraviolet, X-rays, gamma
   3. know the colors of the visible spectrum from low energy to high energy: red, orange, yellow, green, blue, indigo, violet
   4. wavelength and frequency are inversely proportional
   5. wavelength and energy are inversely proportional
   6. frequency and energy are directly proportional
2. Principle energy levels in an atom
   1. Bohr model of the atom
   2. as principle energy level (n) increases the electron is farther from the nucleus
   3. maximum number of electrons in a principle energy level?
   4. energy sublevels: s, p, d, f
   5. energy of orbitals: s < p < d < f
3. Writing electron configurations
   1. Aufbau principle
   2. Hund's rule
   3. Pauli's exclusion principle
   4. write complete electron configurations
   5. be able to write noble-gas shorthand notations
   6. identify the valence shell and count the number of valence electrons in an atom
   7. draw a Lewis dot diagram for the valence shells of atoms
   8. draw orbital diagrams using boxes and arrows to show the number of paired and unpaired electrons in an atom
4. Atomic Radius
   1. trend on the periodic table
   2. why does the radius increase going down a group of elements?
   3. why does the radius of an atom decrease moving left to right across a period on the table?
   4. positive ions (cations) are smaller in size than the neutral atom
   5. negative ions (anions) are larger in size than the neutral atom
5. Ionization Energy
   1. trend on the periodic table
   2. define ionization energy
   3. why does ionization energy decrease moving down a group of elements?
   4. why does ionization energy increase moving left to right across a period on the table?

Chapter 8

1. electron configurations for ions
2. which electrons are lost when a cation forms
3. define ionic bonding
4. Covalent Bonding
   1. relate bond length, bond energy, and bond order
   2. draw Lewis dot structures for molecules with elements that obey the octet rule
   3. label a covalent bond as polar or nonpolar
   4. define electronegativity

Chapter 9

1. define VSEPR theory
2. distinguish between bonding pairs of electrons and lone pairs
3. classify molecules in the AXE classifications
4. identify the shape (or geometry) of a molecule
5. determine if a molecule is polar or nonpolar
6. identify the type of hybridization on an atom in a molecule
7. how many hybrid orbitals are used in a single bond?
8. how many hybrid orbitals are used in a double bond?
9. how many hybrid orbitals are used in a triple bond?